The vapour pressures of acetone and benzene at 65^oC are 580mmHg and 475mmHg respectively

if 5.8g of acetone is mixed with 15.6g of benzene what is the total vapour pressure at 65^oC

Will this mixture distill at 65^oC? Explain

Please give answer and explanation !

Consider the following reaction: CH4 (g) + 2O2 (g)----------} CO2(g) + 2H20(g) ^Hr= -890 kj

a) is heat absorbed or evolved in the course of the reaction?

b) Calculate the amount of heat trasnferred when 45g of CH4 is decomposed by this reaction at constant pressure.

c) For the given sample of CH4 the enthalpy change on reaction is 66.8 kj. How many grams of H2O are produced?

d) what is the value of ^Hr for the reverse of the previous reaction? How many KJ of heat are released when 27g of H2O reacts completely with CO2to form CH4 and O2 at constant pressure?

Calculate the pH for each case in the titration of 50.0 mL of 0.200 M HClO(aq)0.200 M HClO(aq) with 0.200 M KOH(aq).0.200 M KOH(aq). Use the ionization constant for HClO.HClO.

What is the pH before addition of any KOH?KOH?

pH=pH=

What is the pH after addition of 25.0 mL KOH?25.0 mL KOH?

pH=pH=

What is the pH after addition of 35.0 mL KOH?35.0 mL KOH?

pH=pH=

What is the pH after addition of 50.0 mL KOH?50.0 mL KOH?

pH=pH=

What is the pH after addition of 60.0 mL KOH?60.0 mL KOH?

pH=pH=

https://sites.google.com/site/chempendix/ionization

For the following question, please explain specifically what it is you're doing for each step/where your number is coming from (ex.: 1. calculating molar mass... 2. Diving by moles...etc)... This will help me better understand how to solve the problem... thank you!

1a) Adipic Acid contains 49.84% O, and 6.85% H by mass. What is the empircal formula?

1b) The chemical process of rust is described by the following equation:

4Fe (s) + 3O2 (g) --> 2Fe2O3 (s)

The maximum of rust that can be produced from 56 g Fe and 32 g O2 is?

1. Write chemical equations to illustrate the reactions of bromine with cyclohexane, toluene, chlorobenzene, and cyclohexane (NR if no reaction)

2. What type of reaction is occurring between cyclohexane and potassium permanganate? What is the brown precipitate formed from the reaction?

3. You may have seen some reactions of bromine with toluene. Compare this with your observations of the reaction of bromine with chlorobenzene. Based on the structure of toluene where do you think the reaction occurred (aromatic ring or side chain)? Is this reaction similar to the reaction of bromine with an alkane or an alkene? Explain.

Calculate the pH of the resulting solution if 35.0 mL of 0.350 M HCl(aq) is added to

(a) 45.0 mL of 0.350 M NaOH(aq).

pH=

(b) 25.0 mL of 0.450 M NaOH(aq).

pH=

8A : Consider the titration, 10 mL of NaCN(Ka=4.9X10^-10) with .380M HCl. Calculate pH at 0.0mL HCl, 11.82mL HCl.

8B How many mL HCl is needed to reach the equivalence point and what is the pH at this point?

For the following procedure, write a balanced chemical equation for each reaction. Make sure you include the state of matter (s,aq,g,l) and the type of reaction (decomposition, synthesis, single displacement, double displacement, combustion).

Reaction 1
a. Dip one end of a Q-tip in CONCENTRATED hydrochloric acid.
b. Dip one end of a second Q-tip in CONCENTRAED ammonium hydroxide solution.
c. Record initial observations. Caution: Do not observe reaction close to your eyes.
d. Bring the Q-tips close to one another BUT do not let them touch.
e. After you record your observations, flush with water, wrap in a paper towel, and throw in the trash can.

Reaction 2
a. Place a small piece of potato to a small beaker. PLEASE DO NOT WRITE “POTATO” AS A
REACTANT! There is an enzyme in the potato that acts as a catalyst – do research at home to
determine what this enzyme is!
b. Cover the potato with 3% hydrogen peroxide in the beaker.
c. Clean up your station – decant the solution and throw solid contents of beaker into garbage can,
rinse the beaker. Be sure lab table is clean.

True or False

The citric acid cycle consumes more energy than it produces.

The magnesium in a series of soil samples was characterized by atomic absorption spectrometry (AAS). The instrument was calibrated with a series of standards: 0, 50.00, 100.00, 250.00 mg/L MgSO47H2O. These samples produced average instrument readings of 0.005; 0.192 ; 0.401 ; and 0.993. Triplicate analysis of an unknown yielded instrument readings of 0.328, 0.340, 0.335. What is the average concentration and standard deviation of the unknown? Report your answer as ppm Mg. THE OPTION IS NOT 211

what is the boiling point of Hoveyda-Grubbs 2^nd Generation Catalyst?

Chapter 19, Question 2Determine the oxidation state of the transition metal in each compound.

a) NiSO4

b) KMnO₄

c) (NH₄)₂WO₄

d) What is the oxidation state of Pb in PbCrO₄?

e) What is the oxidation state of Cr in PbCrO₄?

f) ZrOCl2.8H2O

PLease Answer all parts of the following:

a) The recommended daily allowance of calcium for men between the ages of 19 to 50 is 1 000 mg Ca. Three multivitamin tablets are analyzed for calcium gravimetrically with the precipitation of calcium cation by oxalate anion. If the mass dry calcium oxalate obtained is 2.0136 g, how many tablets must a man take in a given day to meet the recommended daily allowance? Ca²⁺(aq) + C₂O₄²⁻(aq) ==> CaC₂O₄ (s)

b) Aqueous lead precipitates when mixed with aqueous carbonate.

Pb²⁺(aq) + CO₃²⁻(aq) ==> PbCO₃(s)

If 5.000 g Pb(NO₃)₂and 2.500 g Na₂CO₃are mixed in water, which ion is the limiting reactant? What mass PbCO₃is precipitated? (PbCO₃= 267.21 g/mol, Pb(NO₃)₂= 331.2 g/mol, Na₂CO₃= 105.9888 g/mol)

Write a balanced equation for the oxidation of Co(II) to Co(III) by hydrogen peroxide. Why is this oxidation process assisted by the presence of ammonia?